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A-level Chemistry > Inorganic chemistry and the periodic table > Flashcards

Inorganic chemistry and the periodic table Flashcards

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1
Q

What happens to the atomic radius going down group 2?

A

The atomic radius increases down the group due to the addition of additional shells

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2
Q

What happens to the reactivity going down group 2?

A

The reactivity increases. This is because there is increased electron shielding and increased atomic radius down the group. This makes the 2 outer electrons easier to lose as they have a weaker attraction to the nucleus.

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3
Q

What happens to the ionisation energy going down the group?

A

The first ionisation energy decreases down the group due to a greater atomic radius and increased shielding. This makes it easier for the electron to be removed.

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4
Q

What do group 2 metals react with water to produce?

A

They react with water to produce a metal hydroxide and hydrogen. The metal hydroxide forms as an alkaline solution and is why the group 2 metals are known as the alkaline earth metals.

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5
Q

Mg + 2H20 ->

A

Mg(OH)2 + H2

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6
Q

How does magnesium react with liquid water?

A

very slowly

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7
Q

How can the reaction between magnesium and liquid water be sped up?

A

with steam, as this provides the reaction with extra energy.

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8
Q

What happens when magnesium burns in steam?

A

a bright white flame is produced and hydrogen and magnesium oxide are produced.

(Mg + H20 -> Mg0 + H2)

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9
Q

what happens when group 2 metals react with chlorine?

A

metal chlorides are produced. These are all white precipitates.

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10
Q

Mg + Cl2 ->

A

MgCl2

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11
Q

What happens when group 2 meals react with oxygen?

A

metal oxides are produced

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12
Q

What can strontium and barium react with excess oxygen and heat to form?

A

Metal peroxides

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13
Q

What is the general equation of the reaction between group 2 metals and oxygen?

A

2M + 02 -> 2MO

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14
Q

What is the equation for the reaction between strontium/barium and oxygen?

A

M + 02 -> M02

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15
Q

What do group 2 metals react with dilute acids to produce?

A

bubbles of hydrogen gas and solutions of metal compounds.

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16
Q

X + 2HCl->

A

XCl2 + H2

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17
Q

X + H2S04->

A

XSO4 + H2

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18
Q

X + 2HNO3 ->

A

H2 + X(N03)2

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19
Q

What is HCl?

A

hydrochloric acid

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20
Q

What is H2SO4?

A

Sulfuric acid

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21
Q

what is HNO3?

A

nitric acid

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22
Q

What do group 2 hydroxides react with dilute acid to produce?

A

salt and water. This is a neutralisation reaction

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23
Q

What is the salt formed in neutralisation reactions dependant on?

A

The acid used

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24
Q

what salt does hydrochloric acid form?

A

chloride salts

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25
Q

what salt does sulfuric acid form?

A

sulfate salts

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26
Q

what salt does nitric acid form?

A

nitrate salts

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27
Q

Calcium hydroxide + Hydrochloric acid ->

A

calcium chloride + water

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28
Q

what happens to the solubility of group 2 hydroxides going down group 2?

A

the solubility of the group 2 hydroxides increases going down the group

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29
Q

what happens to the solubility of sulfates going down group 2?

A

the solubility of sulfates decreases down group 2, meaning that magnesium sulfate is the most soluble and barium sulfate is the least soluble

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30
Q

what can barium chloride be used to test for?

A

sulfate ions, as it reacts to form barium sulfate which forms as a white precipitate when sulfate ions are present.

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31
Q

Ba2+ + S042- ->

A

BaS04

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32
Q

do group 2 carbonates and nitrates undergo thermal decomposition to produce solid metal oxides and a variety of gases?

A

yes

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33
Q

what do group 2 carbonates produce when they undergo thermal decomposition?

A

a metal oxide and carbon dioxide

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34
Q

as you go down group 2, is it true that more heat is needed for thermal decomposition ?

A

yes, because the ions increase in size and the carbonates and nitrates increase in thermal stability

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35
Q

what do the group 2 nitrates produce when they undergo thermal decomposition?

A

metal oxide, nitrogen dioxide, oxygen

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36
Q

how can group 1 and group 2 metals be identified?

A

using a flame test

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37
Q

describe the steps for the flame test

A

1) Take a nichrome wire and clean it by placing it into a solution of concentrated hydrochloric acid and then into a blue bunsen burner flame

2) Repeat this cleaning until there is no colour produced in the flame

3) Dip the wire into the unknown metal compound and place it into the flame. Observe the
flame colour produced

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38
Q

what colour does lithium show in the flame test?

A

red

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39
Q

what colour does sodium show in the flame test?

A

orange/yellow

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40
Q

what colour does potassium show in the flame test?

A

lilac

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41
Q

what colour does magnesium show in the flame test?

A

no colour

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42
Q

what colour does calcium show in the flame test?

A

brick red

43
Q

what colour does strontium show in the flame test?

A

crimson red

44
Q

what colour does barium show in the flame test?

A

pale green

45
Q

how can the formation of the colours in the flame test be explained?

A

by electron transitions

46
Q

describe the flame test and electron transitions

A

Electrons exist in orbitals and when energy (such as that supplied by a bunsen burner flame) is absorbed by the species, some electrons will be promoted to orbitals which have a higher energy. The electrons will then drop back down to the original orbital they were in and during this process they release energy, some of which is in the form of light..

The colour produced depends on the wavelength of the light energy emitted. When some electrons drop back down to their original orbital, the energy emitted may not have a wavelength in the visible light part of the electromagnetic spectrum, which explains why not all atoms and ions produce a colour in the flame test.

47
Q

what do group 7 elements need to do in order to gain a full outer shell?

A

they need to gain 1 electron to form a 1- ion

48
Q

why does the atomic radius increase going down group 7?

A

due to the addition of more elctron shells

49
Q

what happens to the electronegativity going down group 7?

A

Electronegativity decreases because the atomic radius and shielding increases. So, electrons in the outer shell are less strongly attracted to the nucleus and so are more easily removed

50
Q

what type of molecules are group 7 elements?

A

Simple covalent molecules that are held together by London forces

51
Q

What happens to the melting/boiling point going down group 7?

A

The melting/boiling points increase. This is because the strength of the London forces increases with the increase in relative atomic mass . This means that more energy is required in order to overcome them

52
Q

What happens to the reactivity going down group 7?

A

The reactivity decreases. This is because as the atomic radius increases, it becomes to gain an electron because the attraction between the nucleus and the electron is weakened due to shielding.

53
Q

Why do the halogens act as good oxidising agents?

A

Because they accept electrons from the species being oxidised and reduced.

54
Q

Why does the oxidising power of the halogens decrease as you go down the group?

A

Because their ability to attract electrons decreases due to shielding and a greater atomic radius

55
Q

What do the relative oxidising strengths mean a halogen will do?

A

the relative oxidising strengths mean a halogen will displace any halide beneath it in the periodic table. Hence, Cl2 will displace Br- and I- ions, and I2 will not displace any halide ions

56
Q

What are halide ions?

A

The negative ions of halogens

57
Q

Why are halide ions good reducing agents?

A

Because they are oxidised and they donate electrons to the species being reduced

58
Q

What happens to the reducing power of halide ions going down group 7?

A

Going down group 7, the reducing power of halide ions increases

59
Q

Why does the reducing power of halide ions reduce going down group 7?

A

Because electrons are easier to lose from larger ions due to shielding and a larger atomic radius

60
Q

What do the redox reactions between group 7 halides and H2SO4 (sulfuric acid) vary depending on?

A

They vary depending on the reducing ability of the halide ion

61
Q

How can the reducing ability of the halide ion be observed?

A

By the relative reactions of the halides with sulfuric acid

62
Q

NaF + H2SO4 ->

A

NaHSO4 + HF

63
Q

NaCl + H2SO4 ->

A

NaHSO4 + HCl

64
Q

Sodium Fluoride + Sulfuric acid ->

A

Sodium Sulfate + Hydrogen fluoride

65
Q

Sodium Chloride + Sulfuric Acid ->

A

Sodium Sulfate + Hydrogen Chloride

66
Q

Will HF and HCl just be observed as misty fumes?

A

Yes

67
Q

NaBr + H2SO4 ->

A

NaHSO4 + HBr (misty fumes)

68
Q

2HBr + H2SO4 ->

A

Br2 + SO2 + 2H20 (orange fumes)

69
Q

The greater the reducing power…..

A

the further the reaction will proceed as the halide is powerful enough to reduce more species

70
Q

What happenes to the reducing power going down group 7?

A

The reducing power increases

71
Q

What happens in a disproportionation reaction?

A

A substance is both oxidised and reduced

72
Q

What does chlorine react with cold water to produce?

A

to produce chlorate(I) ions (ClO - ) and chloride ions via a disproportionation reaction. The oxidation state goes from zero to both +1 and -1

(Cl2 + H20 -≥ Cl0- + Cl- + 2H+)

73
Q

(Cl2 + H20 -≥ Cl0- + Cl- + 2H+)
Where is this reaction used?

A

In water treatment systems where chlorine is used in small quantities to kill bacteria. This poses some risks as chlorine can be toxic ; however the benefits of clean, treated water outweigh the risks

74
Q

Write the equation for the disproportionation reaction between chlorine and cold, dilute sodium hydroxide

A

2NaOH + Cl2 -≥ NaCl0 + NaCl+ H20

75
Q

Write the equation for the disproportionation reaction between chlorine and hot, dilute sodium hydroxide

A

6NaOH + 3Cl2 -≥ 5nacl + NaClO3 + 3H20

76
Q

Do Group 1 and Group 2 metals react with chlorine gas to form metal chlorides?

A

Yes

77
Q

What colour precipitates do metal chlorides form?

A

White

78
Q

When group 2 metals react with chlorine gas is chlorine reduced or oxidised?

A

Chlorine is reduced

79
Q

When group 2 metals react with chlorine gas is the metal reduced or oxidised?

A

The metal is oxidised

80
Q

Mg + Cl2 -≥ MgCl2
What does Magnesium’s oxidation number change to?

A

From 0 to +2

81
Q

Mg + Cl2 -≥ MgCl2
What does Chlorine’s oxidation number change to?

A

From 0 to -1

82
Q

What happens when halide ions are combined with acidified silver nitrate?

A

They form different coloured precipitates. This helps to identify which halide ion is present in a solution

83
Q

What happens when chlorine reacts with acidified silver nitrate (AgNO3)?

A

A white precipitate is formed (AgCl)

84
Q

What happens when bromine reacts with acidified silver nitrate (AgNO3)?

A

A cream precipitate is formed (AgBr)

85
Q

What happens when iodine reacts with acidified silver nitrate (AgNO3)?

A

A yellow precipitate is formed (AgI)

86
Q

What happens when chlorine reacts with dilute ammonia?

A

The precipitate dissolves

87
Q

What happens when bromine reacts with dilute ammonia?

A

There’s no change - precipitate remains cream

88
Q

What happens when iodine reacts with dilute ammonia?

A

There’s no change - the precipitate remains yellow

89
Q

What happens when chlorine reacts with concentrated ammonia?

A

The white precipitate dissolves

90
Q

What happens when bromine reacts with concentrated ammonia?

A

The precipitate dissolves

91
Q

What happens when chlorine reacts with concentrated ammonia?

A

There’s no change, the precipitate remains white

92
Q

What do hydrogen halides react with ammonia gas to form?

A

Ammonium salts

93
Q

HCl + NH3 -≥

A

NH4Cl

94
Q

HBr + NH3 -≥

A

NH4Br

95
Q

HI + NH3 -≥

A

NH4I

96
Q

What do hydrogen halides react with water to form?

A

Dilute acids. In solution, these strong acids dissociate to release their halide ions and hydrogen ions. The hydrogen ions form a hydroxonium ion with water molecules in solution. The resulting solution is acidic .

97
Q

HCl + H2O -≥

A

Cl- + H3O+

98
Q

HBr + h20 -≥

A

Br- + H30+

99
Q

HI + H20 -≥

A

I- + H30+

100
Q

What are sulfate ion (So42-) tested for using?

A

acidified BaCl 2
barium sulfate
which reacts to form a white precipitate of barium sulfate

101
Q

BaCl2 + XSO4 -≥

A

BaSO4 + XCl2

102
Q

Carbonate (CO 3 2- ) and Hydrogencarbonate (HCO 3 - )
When an acid such as HCl is added, the substance containing the carbonate ions will fizz and CO 2
gas is given off . This gas can be collected and bubbled through limewater which will turn
cloudy , confirming its identity as carbon dioxide.

A

XC03 +2HCl -≥ CO2 + H20 + XCl2

103
Q

Ammonium (NH 4
+ )
If ammonium ions are present, adding NaOH and gently warming results in the formation of ammonia gas , which is basic . Therefore, the presence of ammonium ions can be tested by holding damp red litmus paper over a petri dish of the substance being tested. It will turn blue if ammonium ions are present.

A

🖐️

104
Q

Hih

A

Hihi

A-level Chemistry (19 decks)

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